Element "E" belongs to the period 4 and group 16 of the periodic table. The valence shell electron configuration of the element, which is just above ‘E’ in the group is
Select the correct option:
A
$3 s_{n \alpha}^2 3 p^4$
B
$3 d^{10} \cdot 4 s^2, 4 p^4$
C
$4 d^{10} \cdot 5 s^2, 5 p^4$
D
$2 \mathrm{~s}^2, \mathrm{p}^4$
✓ Correct! Well done.
✗ Incorrect. Try again or view the solution.
Solution
$$
E \Rightarrow[\mathrm{Ar}] 3 \mathrm{~d}^{10} 4 \mathrm{~s}^2 4 \mathrm{p}^4
$$
Element above $E \Rightarrow[\mathrm{Ne}] 3 \mathrm{~s}^2 3 \mathrm{p}^4$
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